Assertion : Among the carbon allotropes,diamo | vedclass

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(B) In diamond,each $C$ atom is covalently bonded to four other $C$ atoms to give a tetrahedral unit. Each $C$ atom is $sp^3$ hybridized,and all four

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Both assertion and reason are correct,and the reason is the correct explanation for the assertion

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(B) In diamond,each $C$ atom is covalently bonded to four other $C$ atoms to give a tetrahedral unit. Each $C$ atom is $sp^3$ hybridized,and all four valence electrons are involved in sigma bond formation,leaving no free electrons. Thus,diamond is an insulator.In graphite,each $C$ atom is covalently bonded to three other $C$ atoms in a trigonal planar geometry. Each $C$ atom is $sp^2$ hybridized. Three valence electrons are used in sigma bond formation,while the fourth electron remains in an unhybridized $p$-orbital,which is delocalized over the layers. This free electron makes graphite a good conductor of electricity.Since the difference in electrical conductivity is directly due to the difference in hybridization and the resulting availability of free electrons,the reason is the correct explanation for the assertion.

Assertion : Among the carbon allotropes,diamond is an insulator,whereas,graphite is a good conductor of electricity.
Reason : Hybridization of carbon in diamond and graphite are $sp^3$ and $sp^2$,respectively.

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Assertion : Among the carbon allotropes,diamond is an insulator,whereas,graphite is a good conductor of electricity.Reason : Hybridization of carbon in diamond and graphite are $sp^3$ and $sp^2$,respectively.